Statement-I: `0.02m` solutions of urea and sucrose will freeze at same temperature.
Because
Statement-II: Freezing point of a solution is inversely proportional to the conc. of solution.

Answer

To analyze the statements given in the question, we need to break down the information provided and apply our understanding of colligative properties, specifically the freezing point depression.

### Step-by-Step Solution:

1. **Understanding the Statements**:
- **Statement I**: "0.02m solutions of urea and sucrose will freeze at the same temperature."
- **Statement II**: "Freezing point of a solution is inversely proportional to the concentration of the solution."

2. **Freezing Point Depression**:
The freezing point depression (\( \Delta T_f \)) is given by the formula:
\[ \Delta T_f = K_f \cdot m \]
where \( K_f \) is the freezing point depression constant and \( m \) is the molality of the solution.

3. **Analyzing Statement I**:
- For both urea and sucrose, we have the same molality of 0.02m.
- Since both solutions have the same molality, the freezing point depression for both will be the same, assuming \( K_f \) values for both solutes are similar (which they are for dilute solutions).
- Therefore, the freezing points of both solutions will indeed be the same.

4. **Conclusion for Statement I**:
- Statement I is **True**.

5. **Analyzing Statement II**:
- The freezing point depression is directly proportional to the molality of the solution, which means that as the concentration (molality) increases, the freezing point depression also increases.
- This implies that the freezing point of the solution decreases as the concentration increases, indicating an inverse relationship between freezing point and concentration.
- Therefore, Statement II is also **True**.

6. **Correct Explanation**:
- While both statements are true, Statement II does not correctly explain Statement I. Statement I is true because both solutions have the same molality, not solely because of the inverse relationship mentioned in Statement II.

7. **Final Conclusion**:
- Both statements are true, but Statement II is not the correct explanation for Statement I.

### Summary:
- **Statement I**: True
- **Statement II**: True
- **Explanation**: Statement II is not the correct explanation for Statement I.